Ch12: Acids And Bases
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What are the properties of an acid?
-Conducts electricity -Changes blue litmus to red -Have a sour taste -React with bases to neutralise their properties -React with active metals to liberate hydrogen
What are the properties of a base?
-Conducts electricity -Changes red litmus to blue -Have a slippery feel -React with acids to neutralise their properties -All alkalis, except ammonia, will react with ammonium compounds *Note: base that dissolves in water in called an alkali
What happens when an acid reacts with: 1. Metals 2. Carbonates 3. Alkalis 4. Metal oxides
• Forms hydrogen and a salt • Forms a salt, water and CO2 • Forms a salt and water • Forms salt and water
What is the Arrhenius definition of: 1. An acid 2. Strong acid 3. Weak acid
• A substance that dissociates in water to produce H+ ions • A substance that almost completely dissociates in water to give Hydrogen ions • A substance that only slightly dissociates in water to give hydrogen ions
What are limitations to Arrhenius theory of acids?
-H+ does not exist in water independently (H+ reacts with a water molecule to form a Hydronium (H3O+) ion) -One of the lone pairs of the oxygen atom forms a covalent bond with the proton. Both of the electrons that go into this both originate from oxygen so this is called a dative bond
What is the Arrhenius definition of: 1. A base 2. Strong base 3. Weak base
• Substance that dissociates in water to produce OH- ions • Substance that almost completely dissociates in water to give hydroxide ions • Substance that only slightly dissociates in water to give hydroxide ions
What are the limitations of Arrhenius’s Theory of Acids and Bases?
• Hydronium ions are formed not H+ ions that exist in solution suggested by Arrhenius • Restricted to aqueous solutions (Solvents like liquid ammonia, benzene, methylbenzene are excluded from the definition) • Not all acid-base reactions require water • Not all bases produce OH-
What is the Bronstead-Lowry definition of: 1. An acid 2. Strong acid 3. Weak acid • A base • Strong base • Weak base
• Proton donor • Good proton donor • Poor proton donor • Proton Acceptor • Good proton acceptor • Poor proton acceptor HCl + H2O –> H3O+ + Cl- -HCl donates a proton (acid) -H2O accepts a proton (base)
What are other notes about Bronsted-Lowry theory?
-May be applied to acid-base reactions that do not involve water as the solvent -Water can act as either an acid or a base (Amphoteric- general, Amphiprotic-B/L)
What is a conjugate acid-base pair?
Any pair consisting of an acid and a base which only differ by one proton -A base changes into a conjugate acid when it accepts a proton, vice versa
What can you use to find the pH of any solution?
Universal Indicator
What is neutralisation?
The reaction between an acid and a base to form a salt and water -Rxn between an acid and a base always results in a salt
What is a salt?
The substance formed when the hydrogen ion from an acid is replaced by a metal or an ammonium ion
What are applications of neutralisation?
-Insect stings: -Bee stings are acidic, neutralised with baking soda -Wasp stings are alkaline, neutralised with vinegar -Limestone added to lakes neutralises acidity -Soil treatment: Acidic soil (acid rain) treated with slaked lime, chalk or quicklime -Factory waste: Liquid waste from factories is acidic and must be neutralised using slaked lime before it reaches a river, otherwise sea life will be destroyed